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Module
086
Institution
Third Year / 9th Grade
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CONCEPT DETAILS
KEY CONCEPTS : [ *rating as per the significance of concept]
1. Laws of Chemical Combination ***
2. John Daltons Atomic Theory **
3. Atoms, ions & Chemical Formula ****
4. Mole Concept *****
5. Molar Mass & Avogadro constant ****
Pre requisites
Basic knowledge all states of matter.
Difference in the different states of matter .
SURVEY ANALYSIS
Conceptual levels of comprehension on the basis of feedback taken from the students
Law of Conservation of mass: Law of definite proportion:
proposed by the French chemist proposed by Louis Proust
Antoine Lavoisier (1774) (1799)
Mass can neither be 'A chemical compound
created nor destroyed in a always consists of the
chemical reaction. same elements combined
OR together in the same ratio,
For any chemical process in
a closed system, the mass irrespective of the method
of the reactants must be of preparation or the
equal the mass of the source from where it is
products. taken'.
C + O2 = CO2 One molecule of a compound
water always contains same ratio
12g +32g = 44g of Hydrogen and Oxygen by mass
i.e.
H2O = 2 : 16 = 1 : 8
Verification of “Law of Conservation of mass”
A solution of sodium chloride and silver nitrate are taken separately in the two limbs
of an 'H' shaped tube. The tube is sealed and weighed precisely. The two reactants
are made to react by inverting the tube. The following reaction takes place.
AgNO3(aq) + NaCl (aq) AgCl (s) + NaNO3 (aq)
The whole tube is kept undisturbed for sometime so that the reaction is complete.
When the tube is weighed again it is observed that:
Weight before the reaction = Weight after the reaction
Limitation of “Law of definite proportion”
This law does not hold good when the compound is obtained by using different
isotopes of the combining elements .
Q.1 Why chemical reactions are in accordance with the Law of conservation of mass?
Q.2 Calculate the ratio of atoms present in 5 g of magnesium and 5 g of iron.
[Atomic mass of Mg=24 u, Fe=56 u]
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